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When there is increased pressure, the reaction will favor whichever direction has fewer moles of product. For example, for the reaction Cl2 <-> 2Cl, if the pressure were increased at equilibrium, the reverse reaction would be favored since there is only one mole of Cl2 for every two moles of 2Cl.
An increase in pressure will favor the side of the reaction with less moles of gas and an decrease in pressure will favor the side of the reaction with more moles of gas. However, if an inert gas is added to the system, there is no change in the reaction.
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